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### Course: Chemistry archive>Unit 10

Lesson 6: Electrolytic cells and electrolysis

# Quantitative electrolysis

Calculating how much zinc deposits on the zinc electrode after 1.0 h when a current of 5.0 A is applied to the battery.  Created by Jay.

## Want to join the conversation?

• Can anybody clarify this for me?

In electrolytic cell :-
ANODE - is the source of electron --> hence losses e- and becomes oxidation.
CATHODE - gains e- (from external battery) and becomes a reduction.

• Yes correct. You can also think of OIL/RIG of electrons : Oxidation Is Loss / Reduction Is Gain
• How did you get to 96,500?
charge on single electron = 1.6 * 10^-19 C (e)
charge on one mole electron = e * N.A
= e* 6.022 * 10^23 = 96352 ??
• 6.0221 × 10²³ electrons × 1.6022 × 10⁻¹⁹ C/electron = 96 486 C.
He used a rounded-off number.
• what if the moles of Cu 2+ formed were asked for the same data, would they be the same as that of Zn?
• In this equation one mole of oxidised Cu (from solid to liquid) is needed to reduce one mole of Zn (from liquid to solid). So the molarities are the same however because Cu has slightly different molar mass than Zn the solid Cu bar would be only 6,0 g lighter.
• why is anode attract electrons even tho it positive
• i know its useless to reply to your comment 4 years later, but isnt it the basics to know that the anode always attracts negatively charged ions (anions) and the cathode attracts positive ions (cations)
• Why is electrochemical series not according chemical reactivity in periodic table?
• What's the point of an electrolytic cell? Isn't it just a waste cuz you're using a battery to make a battery? Thanks.
• In an electrolytic cell, isn't there only one cell and no salt bridge?
(1 vote)
• Can't we solve this question in this manner:
Q=5×60×60=18000 Coulumbs
Then,
2 mol of e- gives 1 mol of Zn+2 Zn=65g
So,
2×96,500=193000